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Chemistry--SCH3U > Unit 1-- Matter, chemical trends, & chemical bonding > Flashcards

Unit 1-- Matter, chemical trends, & chemical bonding Flashcards

(98 cards)

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1
Q

What is all matter composed of?

A

Atoms

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2
Q

What are the 3 sub-atomic particles?

A

Protons, Neutrons, and Electrons

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3
Q

How are ions formed?

A

When an atom gains or loses an electron, it becomes an ion and is no longer neutrally charged

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4
Q

ions

A

Charged atoms

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5
Q

Define ISOELECTRONIC

A

Atoms/Ions that have the same number of electrons

same number of valence electrons.

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6
Q

ANION

A

An atom that gains electrons becomes NEGATIVELY charged

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7
Q

CATION

A

An atom that loses electrons and becomes POSITIVELY charged

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8
Q

Two or more forms of the same element that have the same number of protons but a different number of neutrons

A

ISOTOPES

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9
Q

Can differ in mass and there can be heavy and light forms of an element

A

ISOTOPES

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10
Q

ELECTRON PAIRS

A

Two electrons interact in a unique way, allowing them to be situated close to each other

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11
Q

UNPAIRED ELECTRONS

A

Electrons that are in an unfilled outer shell and do not have pairs.
They are more likely to participate in atom bonds

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12
Q

ATOMIC MASS UNIT

A

U
a measure of its atomic mass.
it is one-twelfth of the carbon-12 atom

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13
Q

BETA PARTICLE

A

High energy particles that are negatively charged, and are ejected from the nucleus when the nucleus is unstable and unbalanced

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14
Q

AVERAGE ATOMIC MASS

A

The average of the masses of all the elements isotopes

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15
Q

How are BETA particles formed?

A

emitted from an atom’s nucleus during radioactive decay.

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16
Q

RELATIVE ATOMIC MASSES

A

The weight in grams of the number of atoms of the element contained in 12.00 g of carbon-12

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17
Q

STRONG NUCLEAR FORCE

A

the force that holds protons and neutrons together.

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18
Q

RADIOSOTOPES

A

Isotopes with unstable nuclei that decay into different, often more stable isotopes

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19
Q

ISOTOPIC ABUNDANCE

A

The percentage of atoms with a specific atomic mass found in an element

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20
Q

How many isotopes is CARBON made of

A

2!

Carbon-12 & Carbon-13

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21
Q

What holds the nucleus ( protons and neutrons) together

A

STRONG NUCLEAR FORCE

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22
Q

ENERGY LEVELS

A

fixed distances from the nucleus of an atom where electrons may be found

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23
Q

BOHR MODEL

A

consists of a small, dense nucleus surrounded by orbiting electrons.

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24
Q

LEWIS DOT DIAGRAMS

A

use dots to represent valence electrons around an atomic symbol.

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25
OUTERMOST ELECTRONS
VALENCE ELECTRONS
26
1st energy level
Holds 2 electrons
27
2nd energy level
Holds 8 electrons
28
3rd energy level
Holds 8 electrons
29
OCTET RULE
This tendency to gain or lose electrons is called the
30
PERIODIC LAW
A statement that describes the repeating nature of the properties of the elements
31
PERIOD
Rows on the periodic table of elements
32
GROUP
Columns on the periodic table of elements
33
METALLOIDS
Along both sides of the staircases and demonstrate both metal and non-metal properties
34
HALOGENS
-Many are are liquids or gases - Very poisonous - Reactivity increases UP the group
35
NOBLE GASES( INERT GASES)
-- All are gases - Do not react with anything
36
ALKALINE EARTH METALS
- Solids -React with metals less dramatically than less active metals -Reactivity increases DOWN the group
37
ALKALI METALS ( ACTIVE METALS)
- Solids - Very reactive and reacts violently with water - Reactivity increases DOWN the group
38
When elements are arranged by atomic number, their chemical and physical properties recur periodically
PERIOD LAW
39
ATOMIC RADIUS
the total distance from the nucleus of an atom to the outermost orbital of its electron.
40
TRANSITION METALS
Thier electron configuration is more complex than main-group elements They make the periodic table 18 columns wide
41
SHIELDING..
the outer electrons are shielded and thus have less grip on the nucleus.
42
*ATOMIC SIZE/ RADIUS
As you go down each GROUP in the periodic table, the size of an atom INCREASES As you go across each group on the table the size decreases
43
**ATOMIC SIZE/ RADIUS
As you go ACROSS A PERIOD, the size of an atom DECREASES
44
IONIZATION ENERGY
The energy that is required to REMOVE an electron
45
Tends to DECREASE down a group
IONIZATION ENERGY
46
Tends to INCREASE across a period
IONIZATION ENERGY
47
ELECTRON AFFINITY
The energy associated with the ADDITION of an electron to a neutral atom
48
Tends to DECREASE down a group and increase across a period
ELECTRON AFFINITY
49
ELECTRONEGATIVITY
The measure of an atom's ability to attract electrons in a chemical bond
50
Electronegativity INCREASES up a group across a period
Yes :)
51
EFFECTIVE NUCLEAR CHARGE
The apparent nuclear charge, as experienced by the outermost electrons of an atom, as a result, shielding occurs
52
ATOMIC RADIUS
The distance from the centre of an atom to the boundary within the electrons
53
PERIODIC LAW
When elements are arranged in order of increasing atomic number, there is a periodic repetition of their chemical and physical properties.
54
Metals vs Non-metals
*METALS* -Left side of the staircase -Most are solid and shiny -Good conductors of heat and electricity -tend to LOSE electrons and become positive ions *NON-METALS* -On the right side of the staircase -Many are liquids and gases -poor conductors (good insulators) of heat and electricity Tend to gain electrons and become negative ions
55
IONIC BONDING
In an IONIC BOND electrons are transferred from a metal to a NON-metal
56
COVALENT BONDING
A COVALENT BOND is formed when a pair of electrons are paired between 2 or more non-metals
57
ELECTRONEGATIVITY (EN)
The measure of an atom's ability to attract electrons in a chemical bond it increases up a group and across a period
58
Only non-metals form covalent bonds
:)
59
What do covalent bonds form?
MOLECULES!
60
IONIC COMPOUNDS VS MOLECULAR COMPOUNDS
*IONIC COMPOUNDS* -Crystalline Solids -High melting points -conduct electricity -most have high solubility in water *MOLECULAR COMPOUNDS* -Solids, Liquids, gases -Low melting point -Does not conduct electricity Low solubility in water
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^EN= >1.7
IONIC
62
^EN between 0.5-1.7
POLAR COVALENT
63
^EN between 0-0.4
SLIGHTLY POLAR COVALENT
64
^EN=0
NON POLAR COVALENT ( PURE COVALENT)
65
SINGLE BOND
A covalent bond that results from atoms sharing one pair of electrons
66
DOUBLE BOND
A covalent bond where atoms share two pairs of electrons
67
TRIPLE BOND
A covalent bond where atoms share three pairs of electrons
68
LONE PAIR
A pair of electrons that's not part of a covalent bond
69
LEWIS STRUCTURE
a very simplified representation of the valence shell electrons in a molecule Lewis dot diagram
70
OCTET RULE
When bonds form between atoms, the atoms gain or lose electrons or share electrons, that way they create a filled outer shell containing 8 electrons
71
When two atoms form a bond...
each atom attracts the other atom's electron as well as its own
72
How to calculate ATOMIC MASS
Calculate the average atomic mass using the atomic masses of each isotope and their percent abundances.
73
How to calculate ISOTOPIC ABUNDANCE
Calculate the average atomic mass using the atomic masses of each isotope and their percent abundances
74
Note
Electron negativity increases as the size of the atom decreases
75
Binary Compound
An ionic compound that consists of only two ( bi) elements
76
Naming Ionic Compounds
Metal comes first and non-metal gas comes second but the ending is changed to "ide"
77
Transition Metals
Stock system-- Roman numerals are used to indicate ionic charge "ic" and "ous"-- endings- only applied to some transition metals that only have 2 possible ionic charges
78
BINARY IONIC COMPOUND
contains an ion that is a metal (cation) and an ion that is a nonmetal (anion).
79
ALKALI
A base that is soluble in water
80
OXOACIDS
An acid composed of hydrogen, oxygen, and atoms of at least one other element
81
STRUCTURAL FORMULA
A diagram that has the chemical symbols connected by lines to show the connections among atoms in a chemical compound
82
NAMES/STRUCTURES FOR MOLECULAR COMPOUNDS
1. MONO 2. DI 3. TRI 4. TETRA 5. PENTA 6. HEXA 7. HEPTA 8. OCTA 9. NONA 10. DECA EG. S,F6--> sulfur *HEXA*fluoride
83
POLYATOMIC IONS/ RADICALS
Ions that are composed of more than one element are called polyatomic ions
84
ACIDS VS BASES
*ACIDS* - Taste sour -Conducts electricity in aqueous solutions -turns litmus paper RED -Feels wet -Reacts with some metals to form H2 (g) -Reacts with carbonates to form CO2 *BASES* -Taste Bitter -Conducts electricity in aqueous solutions Turns litmus paper BLUE -Feels slippery -Does not react with metals -Does not react with Carbonates
85
1 O (oxygen) more--SO5^-2
*PER*sulfate
86
MOST COMMON --> SO4^-2
SULFATE
87
1 O less --> SO3^-2
sulfI*ITE*
88
2 O Less --> SO2^-2
*HYPO*sulf*ITE*
89
ACIDS
*ACIDS* - Taste sour -Conducts electricity in aqueous solutions -turns litmus paper RED -Feels wet -Reacts with some metals to form H2 (g) -Reacts with carbonates to form CO2
90
BASES
*BASES* -Taste Bitter -Conducts electricity in aqueous solutions Turns litmus paper BLUE -Feels slippery -Does not react with metals -Does not react with Carbonates
91
ACID & BASE NOMENCLATURE BASES
Bases are IONIC COMPOUNDS eg. KOH - Potassium hydroxide Na OH - Sodium hydroxide
92
BASES
Ionic Compounds eg. KOH --potassium hydroxide
93
TWO TYPES OF ACIDS
**Binary acids & Oxyacids**
94
1. BINARY ACIDS
H*X* where *X* is the nonmetal ( usually a halogen) you must state the *HYDRO* first, and then end the nonmetal's name with an "ic" ending and the word "acid" eg. HF-- Hydrofluoric acid HCl-- Hydrochloric acid
95
ORDER OF BINARY ACIDS
H*X* ( *X* is nonmetal) 1. state HYDRO 2. end the nonmetal with "ic" 3. end with the word "acid"
96
2. OXYACIDS
- Contain *H* and a polyatomic ion ( that contains o) - Use the beginning of the polyatomic ion name add an "ic" ending - Add the word "acid" eg. HNO3-- Nitric acid Sulfuric acid --> H2,SO4
97
- Contain *H* and a polyatomic ion ( that contains o) - Use the beginning of the polyatomic ion name -add an "ic" ending - Add the word "acid"
OXYACIDS
98
Different Oxyacids can be found by changing the number of oxygen atoms contained in the polyatomic ion
1 O (oxygen) more-- H2 SO5 -- *PER*sulfuric acid Most common-- H2 S04 -- sulfuric acid 1 O less-- H2 SO3 -- H2 SO3 --sulfur*OUS* acid 2 O less-- H2 SO2 -- *HYPO*sulfur*OUS* acid

Chemistry--SCH3U (4 decks)

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